Identify the correct Lewis structure of H3O+. Ensure that all charges and lone pairs are shown.

Question

Identify the correct Lewis structure of H3O+. Ensure that all charges and lone pairs are shown.

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Question restatement: Identify the correct Lewis structure of H3O+ and ensure charges and lone pairs are shown.

Since the answer options provided are blank, I will reason generally about the correct Lewis structure and common incorrect possibilities, so you can recognize the right structure if you see it.

Key facts to apply:
- Hydronium ion H3O+ consists of an oxygen atom covalently bonded to three hydrogen atoms.
- Oxygen brings 6 valence electrons; each O–H bond uses 2 electrons, and there are three such bonds, totaling 6 electrons used in bonding.
- The overall species has a +1 formal charge because there are 9 valence electrons from H (3) and O (6) combined, but the structure uses only 8 electrons around the atoms (one electron less than neutral count), which corresponds to a +1 charge on the molecule.
- The correct arrangement places a lone pair on the oxygen (to complete its octet after forming three bonds), resulting in three single bonds and one lone pair on O, with the overall +1 charge on the molecule.

Option analysis (typical possibilities you might see):
- Correct structure: O in the center with three O–H single bonds and one lone pair on O, and a +1 formal charge on O (often depicted as [H–O(H)–H] with one lone pair on O and a + sign on the molecule or explicitly as O with a +1 charge). This satisfies: O has 3 bonds (6 electrons) plus 2 electrons in the lone pair = 8 electrons around O, and the molecule carries a +1 charge overall.
- Common incorrect option A (e.g., O with four bonds or no lone pair on O): This would make oxygen hypervalent (four bonds) or fail to place a lone pair, which would misrepresent octet rules and the electron count, and it would disrupt the molecule’s formal charge balance.
- Common incorrect option B (e.g., H atoms attached in a way that assigns a positive charge to H or omits the positive charge entirely): In H3O+, hydrogen atoms are neutral, so assigning a positive charge to H would be incorrect; the +1 charge must reside on the oxygen due to its electron count relative to valence.
- Common incorrect option C (e.g., no lone pairs on O): O needs a lone pair to complete the octet after forming three bonds; omitting the lone pair would give an incomplete octet and an incorrect depiction of electron distribution.
- Common incorrect option D (e.g., inconsistent number of hydrogens around O): H3O+ specifically has three hydrogens bonded to O; any structure showing a different number of O–H bonds would violate the chemical formula and the known geometry of hydronium.

In summary, the correct Lewis structure must show a central oxygen with three single bonds to hydrogen atoms, one lone pair on oxygen, and a formal +1 charge on the molecule (typically on the oxygen). Any option that assigns the charge to hydrogen, lacks the oxygen lone pair, or miscounts bonds around oxygen would be incorrect.

CHEM1011 (ND) Lecture quiz: Week 6

Identify the correct Lewis structure of H3O+. Ensure that all charges and lone pairs are shown.

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